Freezing Point Depression
A solution freezes at a ______ temperature than that of the pure
solvent.
What is lower
DeltaT=
What is miKb
The M in pi=MRT
What is Molarity
The partial pressure exerted by any component of an "ideal" solution is equal to the vapor pressure of the pure component multiplied by its mole fraction.
What is Raoult's Law
The ions formed when C6H12O6 dissolves in water
No ions form as glucose does not dissociate.
True or false:
The change in Freezing point is a positive value.
What is true
A liquid typically boils at 200 °C. If an insoluble salt is added to the liquid, its new boiling point will be
What is 200 °C
The units for the gas law constant
L*atm/mol*K
Adding a nonvolatile solute to a pure solvent will does this to the solvent’s
vapor pressure
What is lower
Substances that dissolve in water and undergo a physical or chemical change to produce ions
What are Electrolytes
Assuming ideal solution behavior, what is the freezing point of a 1.85 m solution of a nonvolatile nonelectrolyte solute in nitrobenzene?
Kf=8.1
FP=5.67
What is −9.3 °C
Calculate the molality of each of the following solutions:
0.372 g of tetrahydropyridine, C5H9N, in 125 g of chloroform, CHCl3
What is 0.0358 m
M= (moles of solute)/(Liters of solution)
True or false:
Mol fraction is dependent on temperature
What is False
Substances that do not produce ions when
dissolved in water.
What is a nonelectrolyte
Estimate the freezing point of a permanent type of antifreeze solution made up of 100.0 g ethylene glycol, C2H6O2 (MM = 62.07) and 100.0 g H2O (MM = 18.02). The kf = 1.86° C/m
What is -30 degrees C
Calculate the boiling point elevation of 0.100 kg of water containing 0.010 mol of NaCl, 0.020 mol of Na2SO4, and 0.030 mol of MgCl2, assuming complete dissociation of these electrolytes and ideal solution behavior.
What is
0.870 °C
Assuming ideal solution behavior, what is the osmotic pressure (atm) a solution with a volume of 0.750 L that contains 5.0 g of methanol, CH3OH, in water at 37 °C?
R=0.08206 L*atm/mol*K
What is 5.3 atm
Calculate the mole fraction of the solute and solvent:
25 g of Cl2 in 125 g of dichloromethane, CH2Cl2
What is
XCl2=0.192;
XCH2CI2=0.808;
Ca(NO₃)₂ has a van't Hoff factor of i = 2.50. What is the concentration of particles in a 0.991 M solution of Ca(NO₃)₂?
2.48M
Assuming ideal solution behavior, what is the freezing temperature of a solution of 115.0 g of sucrose, C12H22O11, in 350.0 g of water?
What is −1.8 °C
A solution containing 5.00 g of a compound dissolved in 25.00 g of carbon tetrachloride (bp 76.8 °C; Kb = 5.02 °C/m) exhibits a normal boiling point of 81.5 °C. Assuming ideal solution behavior, what is the molar mass of the compound?
What is 2.1 × 102 g mol−1
The osmotic pressure of human blood is 7.6 atm at 37 °C. What mass of glucose, C6H12O6, is required to make 1.00 L of aqueous solution for intravenous feeding if the solution must have the same osmotic pressure as blood at body temperature, 37 °C (assuming ideal solution behavior)?
What is 54g
A solution contains 5.00 g of urea, CO(NH2)2, a nonvolatile compound, dissolved in 0.100 kg of water. If the vapor pressure of pure water at 25 °C is 23.7 torr, what is the vapor pressure of the solution (assuming ideal solution behavior)?
What is 23.4
Which has the largest Van't Hoff factor?
1) Li2SO4
2) KI
3) Na3PO4
4) C6H12O6
What is
3) Na3PO4; i=4